Answer:
CuSO4·xH2O is a hydrated copper(II) sulfate compound where x represents the number of water molecules associated with each copper(II) sulfate molecule.
To determine the value of x, we need some additional information, such as the mass of the hydrated compound or the percentage of water by mass.
For example, if we have the mass of the hydrated compound, we can use it to determine the mass of copper(II) sulfate and the mass of water. Then, we can use the molar mass of CuSO4 and H2O to calculate the number of moles of each substance. Finally, we can use the molar ratios to find the value of x.
Let's take an example: suppose we have 5 grams of CuSO4·xH2O and upon heating, we found that 1.25 grams of water is lost. We can use this information to calculate the value of x as follows:
Calculate the mass of copper(II) sulfate:
mass of CuSO4 = mass of CuSO4·xH2O - mass of water lost
mass of CuSO4 = 5 g - 1.25 g
mass of CuSO4 = 3.75 g
Calculate the number of moles of copper(II) sulfate:
moles of CuSO4 = mass of CuSO4 / molar mass of CuSO4
moles of CuSO4 = 3.75 g / 159.61 g/mol (molar mass of CuSO4)
moles of CuSO4 = 0.0235 mol
Calculate the number of moles of water:
moles of H2O = mass of water lost / molar mass of H2O
moles of H2O = 1.25 g / 18.02 g/mol (molar mass of H2O)
moles of H2O = 0.0693 mol
Use the molar ratio of CuSO4 to H2O to find the value of x:
moles of H2O / moles of CuSO4 = x
0.0693 mol / 0.0235 mol = x
x = 2.95
Therefore, in this example, the value of x is approximately 2.95, which means that each copper(II) sulfate molecule in the hydrated compound is associated with approximately 2.95 water molecules
Step-by-step explanation:
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